7.3 Hydrogen Atom The Bohr model of the hydrogen atom served as a major step tow

Question

7.3 Hydrogen Atom

The Bohr model of the hydrogen atom served as a major step toward describing the structure of atoms. It is essentially a classical model with one quantum modification, namely the orbital angular momentum of the electron is an integer multiple, n, of Planck's constant, h, divided by 2*pi. That is L=rmv=n(h/(2*pi)).

An electron in a hydrogen atom transitions from state n to state n-2. Find a general formula for the frequency of the emitted light for this transition. Does your formula predict the same energy regardless of the initial value of n? What does this mean regarding the

Explanation / Answer

The smaller the energy the longer the wavelength..

In the hydrogen atom, with Z = 1, the energy of the emitted photon can be found using:

E = (13.6 eV) [1/nf2 - 1/ni2]

Atoms can also absorb photons. If a photon with an energy equal to the energy difference between two levels is incident on an atom, the photon can be absorbed, raising the electron up to the higher level.

For a photon E = hf = hc/lambda

The angular momentum (mvr) of electron in nth orbit is equal to nh/2?.

nh/2? gives angular momentum of electron revolving in a circular orbit as proposed by Neils Bohr

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